Sulfur has six electrons in its outer most energy level. In ionic bonding, it would tend to _____________________________.
A.
take on two more electrons
B.
give away two electrons
C.
give away six electrons
D.
not take on anymore electrons
The answer is A
To determine the answer to this question, we need to understand how ionic bonding works. Ionic bonding occurs when atoms transfer electrons from one atom to another, resulting in the formation of ions. In this process, each atom aims to achieve a stable electron configuration, typically by filling its outermost energy level.
Sulfur has six electrons in its outermost energy level. To achieve a stable configuration, sulfur can either gain electrons to fill its outermost shell or lose electrons to empty its outermost shell.
Looking at the options given:
A. Taking on two more electrons would give sulfur a total of eight electrons in its outermost energy level, achieving a stable electron configuration. This would most likely lead to the formation of a sulfide ion.
B. Giving away two electrons would leave sulfur with only four electrons in its outermost energy level, which is not a stable configuration. This option is unlikely as sulfur tends to gain electrons rather than lose them.
C. Giving away all six electrons would leave sulfur with no electrons in its outermost energy level, which is not a stable configuration. Sulfur is more likely to gain electrons rather than losing all of them.
D. Not taking on any more electrons would not help in achieving a stable electron configuration. Sulfur needs to either gain or lose electrons to reach a stable state.
Based on this analysis, the most appropriate answer is option A. Sulfur would tend to take on two more electrons in ionic bonding.